Hey Guys so I have this problem with ICE tables that is extremely confusing for me so I would love some help on it!

Question

At a Certain Temperature, the equilibrium constant for the reaction of NO with Cl2 is 6250. If the initial concentration of NOCl is 1.0M and that of NO 0.10M what is the concentration of Cl2 at equilibrium?

2NO(g)+ Cl2(g)<-->2NOCl(g)

a) 1.0M
b) 0.062 M
c) 0.0016 M
d) 0.016 M
Anything Helps!

Answer 1

What's the (Cl2) initially. I've used 0 below.
......2NO(g)+ Cl2(g)<-->2NOCl(g)
I.....0.1M.....0........1.0M
C.....2x +x -2x
E.....0.1+2x...x........1-2x

Substitute the E line into Kc expression and solve for x. This is a cubic equation.

Answer 2

I think you made a typo for answer D. Are you sure that isn't 0.0106
By the way, instead of solving a cubic equation you can substitute each of the answers into the expression an see which comes out with K of 6250